PHYSICAL CHEMISTRY
By: Shailendra Kumar
PHYSICAL CHEMISTRY
by:
SHAILENDRA KR.
Meq. Approach
Classes at: SCIENCE TUTORIALS; Opp. Khuda Baksh Library, Ashok Rajpath, Patna
PIN POINT STUDY CIRCLE; House No. 5A/65, Opp. Mahual Kothi, Alpana Market, Patna
Topic: Chemical Equilibrium
01.
02.
03.
04.
2 mole of PCl 5 were heated in a closed
vessel of 2 litre capacity. At equilibrium 40%
of PCl5 dissociated into PCl3 and Cl2. The
value of equilibrium constant is:
(a) 0.267
(b) 0.53
(c) 2.63
(d) 5.3
One mole of ethyl alcohol was treated with
one mole of acetic acid at 25°C.
2/3 of the acid changes into ester at
equilibrium. The equilibrium constant for the
reaction will be :
(a) 1
(b) 2
(c) 3
(d) 4
1.
2.
07.
2NO2, α is degree
If in the reaction N2O4
of dissociation of N2O4 then the number of
molecules at equilibrium will be:
(a) 3
(b) 1
(c) (1–α)2
(d) (1+α)
CuSO4⋅3H2O(s) + 2H2O (v)
If CuSO4⋅5H2O
K p =1.086 × 10 –4 atm 2 at 25°C. The
efflorescent nature of CuSO4⋅5H2O can be
noticed when vapour pressure of H2O in
atmosphere is:
(a) > 7.92 mm
> 7.92 mm
(c) <
05.
06.
(b) < 7.92 mm
08.
09.
(d) None of these
Sulphide ions in alkaline solution react with
solid sulphur to form polyvalent sulphide ions.
The equilibrium constant for the formation of
S22– and S32– from S and S2– ions are 1.7 and
5.3 respectively. Equilibrium constant for the
formation of S32– from S22– and S is:
10.
(a) 1.33
(b) 3.11
(c) 4.21
(d) 1.63
When 20 g of CaCO3 were put into 10 litre
flask and heated to 800°C, 35% of CaCO3
remained unreacted at equilibrium. Kp for
decomposition of CaCO3 is:
(a) 1.145 atm
(b) 0.145 atm
(c) 2.145 atm
(d) 3.145 atm
1.1 mole of A are mixed with 2.2 mole of B
and the mixture is then kept in one litre flask
till
the
equilibrium
is
attained
A + 2B
2C + D. At the equilibrium, 0.2
mole of C are formed. The equilibrium
constant of the reaction is:
(a) 0.001
(b) 0.002
(c) 0.003
(d) 0.004
In a chemical equilibrium, the rate constants
of the forward and backward reactions are
respectively 3.2 × 10–4 and 1.2 × 10–5, the
equilibrium constant is:
(a) 0.37
(b) 26.7
(c) 0.25
(d) 3.7
2NO(g) + O2 (g),
For the reaction, 2NO2 (g)
Kc = 1.8 × 10–6 at 185°C. At 185°C, the Kc for
NO (g) + 1/2 O2 (g)
NO2 (g) is :
(a) 0.9 × 106
(b) 7.5 × 102
(c) 1.95 × 10–3
(d) 1.93 × 103
4 mole of A are mixed with 4 mole of B, when
2 mole of C are formed at equilibrium,
according to the reaction, A + B
C + D.
The equilibrium constant is:
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PHYSICAL CHEMISTRY
11.
12.
13.
(a) 4
(b) 1
(c) √2
(d) √4
2HI (g) at
For the reaction, H2 (g) + I2(g)
720 K, the value of equilibrium constant is
50, when equilibrium concentration of both
H 2 and I 2 is 0.5 M.K p under the same
conditions will be:
(a) 0.02
(b) 0.2
(c) 50
(d) 50RT
At a given temperature, the Kc for the reaction,
PCl5 (g) PCl3 (g) + Cl2 (g) is 2.4 × 10–3. At
the same temperature, The Kc for the reaction
PCl3 (g) + Cl2 (g) PCl5 (g) is :
(a) 2.4 × 10–3
(b) – 2.4 × 10–3
(c) 4.2 × 102
(d) 4.8 × 10–2
On adding A to the reaction at equilibrium,
AB (s)
A (g) + B (g), the new equilibrium
concentration of A becomes double, the
equilibrium concentration of B would become:
By: Shailendra Kumar
[P 4O10]
(c) Kc = –––––––––
5[P4] [O2]
17.
16.
If
equilibrium
concentration
are
[A] = 0.25, [B] = 0.4 and [C] = 0.5 mol dm–3.
The value of Kc is:
18.
19.
(a) 0.25
(b) 0.4
(c) 2.5
(d) 4.0
At a certain temperature, 2HI
H2 + I2 only
50% HI is dissociated at equilibrium. The
equilibrium constant is:
(a) 1.0
(b) 3.0
(c) 0.5
(d) 0.25
The reaction, A + 2B
2C + D was studied
using an initial concentration of B which was
1.5 more that of A. But the equilibrium
concentration of A and C were found to be
equal. Then the Kc for the equilibrium is :
(a) 4
(b) 8
(c) 1/8 of its original value
(c) 6
(d) 0.32
20.
For a reaction, 2A + B
C, where initial
concentration of A = 2M, B = 1M and
C = 0, the concentration of B at equilibrium
is 0.5 M. The value of equilibrium constant
for the reaction is:
(a) 0.5
(b) 2.0
(c) 1.0
(d) 1.5
For a reaction N2 + 3H2 –––––→ 2NH3; ∆H =
–22 kcal. If energy of activation for this
reaction is 70 kcal, the energy of activation
for backward reaction is :
In a system : A (s)
2B (g) + 3C (g). If the
concentration of C at equilibrium is increased
by a factor 2, it will cause the equilibrium
concentration of B to change to:
(a) two times of its original value
(b) one half of its original value
(c) 2√2 times of its original value
(d) 1/2√2 times of its original value
(a) 70 kcal
(b) 92 kcal
The vapour density of undecomposed N2O4
is 46. When heated, vapour density
decreases to 24.5 due to its dissociation to
NO2. The percent dissociation of N2O4 at the
final temperature is :
(c) 48 kcal
(d) none of these
(a) 87
(b) 60
(c) 40
(d) 70
21.
The equilibrium constant for the reaction;
P4 (s) + 5O2 (g)
1
(a) Kc = ––––––
[O2]5
1.
2.
2C (aq.)
(b) 1/4 of its original value
(d) Twice its original value
15.
Equilibrium is established in the reaction,
A (aq.) + B (aq.)
(a) 1/2 of its original value
14.
[P4O10]
(d) Kc = –––––––––
[P4] [O2]5
P4O10 (s) is :
(b) Kc = [O2]5
22.
For an equilibrium change involving gaseous
phase, the forward reaction is first order while
the reverse reaction is second order. The unit
of Kp for the forward equilibrium is :
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PHYSICAL CHEMISTRY
(b) Atm2
(a) Atm
(c) Atm
23.
By: Shailendra Kumar
–1
(d) Atm
29.
–2
The formation of phosgene is represented
as,
CO + Cl2
COCl2
(a) 2x M
The reaction is carried out in 500 mL flask.
At equilibrium 0.3 mole of phosgene, 0.1 mole
of CO and 0.1 mole of Cl2 are present. The
equilibrium constant of the reaction is:
24.
25.
26.
27.
28.
1.
2.
(a) 30
(b) 15
(c) 5
(d) 3
(b) x M
(c) Between x M and x/2 M
(d) Less than x/2 M
30.
∆Gº for the reaction X + Y
Z is
– 4.606 kcal. The equilibrium constant for the
reaction at 227°C is:
(a) 100
(b) 10
(c) 2
(d) 0.01
The partial pressure of CH3OH(g), CO(g) and
H2(g) in equilibrium mixture for the reaction,
CO(g) + 2H2(g)
CH3OH(g) are 2.0, 1.0
and 0.1 atm respectively at 427ºC. The value
of Kp for the decomposition of CH3OH to CO
and H2 is :
(a) 102 atm
(b) 2 × 102 atm–1
(c) 50 atm2
(d) 5 × 10–3 atm2
The equilibrium constant of a reaction is 20.0.
At equilibrium, the rate constant of forward
reaction is 10.0. The rate constant for
backward reaction is:
(a) 0.5
(b) 2.0
(c) 10.0
(d) 200.0
2CO(g),
For the reaction, C(s) + CO2 (g)
the partial pressures of CO2 and CO are 2.0
and 4.0 atm respectively at equilibrium. The
Kp for the reaction is:
(a) 0.5
(b) 4.0
(c) 8.0
(d) 32.0
PCl 3 + Cl 2, the
In the reaction, PCl3
amounts of PCl5, PCl3 and Cl2 at equilibrium
are 2 mole each and the total pressure is 3
atm. The equilibrium constant Kp is :
(a) 1.0 atm
(b) 2.0 atm
(c) 3.0 atm
(d) 6.0 atm
In an aqueous solution of volume 500 mL,
when the reaction of 2Ag++Cu Cu2+ + 2Ag
reached equilibrium the [Cu2+] was x M.
When 500 mL of water is further added, at
the equilibrium [Cu2+] will be:
31.
32.
40% of a mixture of 0.2 mole of N2 and 0.6
mole of H2 react to give NH3 according to the
2NH3(g) at
equation, N2(g) + 3H2(g)
constant temperature and pressure. Then the
ratio of the final volume to the initial volume
of gases are:
(a) 4 : 5
(b) 5 : 4
(c) 7 : 10
(d) 8 : 5
At temperature T, a compound AB 2 (g)
dissociates according to the reaction
2AB2(g)
2AB(g) + B2(g) with a degree of
dissociation x, which is small compared with
unity. The expression for Kp, in terms of x
and the total pressure P, is:
(a) Px3 / 2
(b) Px2 / 3
(c) Px3 / 3
(d) Px2 / 2
PCl3 (g) + Cl2(g)
Two systems PCl5(g)
and COCl 2 (g)
CO(g) + Cl 2 (g) are
simultaneously in equilibrium in a vessel at
constant volume. If some CO is introduced
into the vessel then at the new equilibrium
the concentration of :
(a) PCl5 is greater
(b) PCl3 remains unchanged
(c) PCl5 is less
33.
(d) Cl2 is greater
Kc for the reaction:
Ag+ + 2CN–, the equilibrium
[Ag(CN)2]–
constant at 25ºC is 4.0 × 10–19, then the silver
ion concentration in a solution which was
originally 0.1 molar in KCN and 0.03 molar in
AgNO3 is:
(a) 7.5 × 1018
(b) 7.5 × 10–18
(c) 7.5 × 1019
(d) 7.5 × 10–19
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PHYSICAL CHEMISTRY
34.
By: Shailendra Kumar
For the reaction A + B 3C at 25ºC, a 3 litre
vessel contains 1, 2, 4 mole of A, B and C
respectively. If Kc for the reaction is 10, the
reaction will proceed in:
is Kc = 4.9 × 10–2. The value of Kc for the
reaction
2SO2(g) + O2(g)
will be
(a) Forward reaction
(b) Backward reaction
(c) In either direction
41.
(d) In equilibrium
35.
36.
The equilibrium constant K c for
A(g)
B(g) is 1.1, Gas B will have molar
concentration greater than 1 if:
(a) (A) = 0.91
(b) (B) > 0.91
(c) (A) > 1
(d) At all these
37.
38.
42.
Amount of PCl5 (in mole) need to be added
to one litre vessel at 250ºC in order to obtain
a concentration of 0.1 mole of Cl2 for the given
change is:
PCl5
(b) 0.0341
(c) 3.415
(d) 0.3145
For the reaction, CO (g) + Cl2(g)
the value of Kp/Kc is equal to:
(a) 1.0
(b) RT
(c) √RT
(d) 1/RT
39.
40.
(d) 2.5 × 10–2
A definite amount of solid NH4HS is placed in
a flask already containing NH3 gas at certain
temperature and 0.50 atm pressure. NH4HS
decomposes to give NH3 and H2S and total
equilibrium pressure in flask is 0.84 atm. The
equilibrium constant for the reaction is:
(a) 0.30
(b) 0.18
(c) 0.17
(d) 0.11
The equilibrium constant for the reaction,
SO3(g)
1.
2.
SO2(g) + 1/2 O2 (g)
For an endothermic reaction where ∆H
represent the enthalpy of the reaction in kJ/
mol, the minimum value for energy of
activation will be:
(a) Less than ∆H
(b) Zero
(c) More than ∆H
(d) Equal to ∆H
Favourable conditions for manufacture of
ammonia by the reaction,
2NH3; ∆H = –21.9 kcal are:
(d) High temperature, high pressure and
catalyst
43.
Predict the conditions for forward reaction
on the basis of Le-Chatelier’s principle for:
2SO2(g) + O2(g)
at room temperature T is 4 × 10–4. The value
of Kc for NO (g)
1/2 N2(g) + 1/2 O2 (g) at
the same T is:
(c) 4 × 10–4
(d) 4.9 × 10–2
(c) High temperature, low pressure and
catalyst
2NO(g)
(b) 50
(c) 9.8 × 10–2
(b) Low temperature, high pressure and
catalyst
COCl2(g)
(a) 0.02
(b) 2.40 × 10–3
(a) Low temperature, low pressure and
catalyst
The equilibrium constant (Kc) for the reaction,
N2 (g) + O2(g)
(a) 416
N2 + 3H2
PCl3 + Cl2; Kc = 0.0414 mol/litre
(a) 0.3415
2SO3(g)
2SO3(g) ∆H = –198 kJ
(a) Lowering the temperature
increasing pressure
and
(b) Any value
pressure
and
of
temperature
(c) Lowering of temperature as well as
pressure
(d) Increasing temperature as well as
pressure
44.
45.
The reaction quotient (Q) at equilibrium is :
(a) = 1
(b) = K
(c) > K
(d) < K
A chemical reaction A
equilibrium when:
B is said to be at
(a) Complete conversion of A to B has
taken place
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PHYSICAL CHEMISTRY
By: Shailendra Kumar
(b) Conversion of A to B is only 50%
complete
46.
47.
(c) Kc = Kp
52.
(d) Kc < Kp
For the chemical reaction,
(c) Only 10% conversion of A to B has
taken place
3X (g) + Y (g) –––––→ X3Y (g); the amount of
X3Y at equilibrium is affected by:
(d) The rate of transformation of A to B
is just equal to the rate of
transformation of B to A in the
system
(a) Temperature and pressure
(b) Temperature only
(c) Pressure only
2NH3; ∆H = –ve then:
For N2 + 3H2
(d) Temperature, pressure and catalyst
53.
(a) Kp = Kc
(b) Kp = KcRT
(c) Kp = Kc(RT)–2
(d) Kp = Kc(RT)–1
Which oxide of nitrogen is the most stable?
(a) 2NO2 (g)
N2 (g) + 2O2 (g);
K = 6.7 × 1016 mol litre–1
On applying pressure to the equilibrium,
Ice
(b) 2NO (g)
water
N2 (g) + O2 (g);
K = 2.2 × 1030 mol litre–1
Which phenomenon will happen?
(c) 2N2O5 (g)
(a) More ice will be formed
2N2 (g) + 5O2 (g);
K = 1.2 × 1034 mol–5 litre–5
(b) More water will be formed
(d) 2N2O (g)
(c) Equilibrium will not be disturbed
2N2 (g) + O2 (g);
K = 3.5 × 1033 mol litre–1
(d) Water will evaporate
48.
Oxidation of SO 2 by O 2 to SO 3 is an
exothermic reaction. The yield of SO3 will be
maximum if:
(a) Temperature is increased
pressure is kept constant
and
(b) Temperature
is
reduced
pressure is increased
and
54.
(a) The reaction has gone to near
completion towards right
(b) The reaction has not yet started
(c) Both temperature and pressure are
increased
(c) The reaction has gone to near
completion toward left
(d) None of the above
55.
(d) Both temperature and pressure are
reduced
49.
50.
N2 + O2
2NO
.........(I)
1/2 N2 + 1/2 O2
(a) Endothermic
(b) Exothermic
(a) K2 = K1
(b) K2 = √K1
(c) Fast
(d) Slow
(c) K1 = 2K2
(d) K1 = 1/2 K2
Which equilibrium in gaseous phase would
be unaffected by an increase in pressure?
2NO2
(c) N2 + 3H2
(b) N2 + O2
2NH3
(d) CO + 1/2 O2
CO2
For the reaction H2 + I2
(a) Kc = 2Kp
1.
2.
If K1 and K2 are equilibrium constants for
reaction (I) and (II) respectively for,
The equilibrium constant Br2 2Br at 500 K
and 700 K are 10–10 and 10–5 respectively.
The reaction is:
(a) N2O4
51.
A higher value for equilibrium constant, K
shows that:
2HI:
(b) Kc > Kp
2NO
NO
.........(II)
Then:
56.
If pressure is applied to the equilibrium of
solid liquid. The melting point of the solid:
(a) Will not change
(b) May increase or decrease depending
upon its nature
(c) Will always increase
(d) Will always decrease
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PHYSICAL CHEMISTRY
57.
58.
By: Shailendra Kumar
(a) 1/9
(b) 1/81
(c) 1/27
(d) 1/3
(b) PCl5 (g)
(d) SOCl2 (g)
63.
CaO (s) + CO2 (g)
proceeds to completion because :
64.
(a) of high temperature
(a) 0
(b) 1
(c) 2
(d) 10
For a system in equilibrium, ∆G = 0 under
conditions of constant:
(b) temperature and volume
(d) of low temperature
(c) Energy and volume
When two reactants A and B are mixed to
give products C and D, the reaction quotient
Q, at the initial stages of the reaction:
(d) Pressure and volume
65.
(b) Favours the backward rate only
(c) Favours both the forward and
backward rates as the case may be
For the reaction,
CuSO4⋅5H2O(s)
(d) Favours neither the forward not
backward rates
CuSO4⋅3H2O(s) + 2H2O(v)
Which one is correct representation?
2
66.
2
(a) Kp = (pH O)
(b) Kc = [H2O]
2
2
(c) Kp = Kc (RT)
(d) All of these
The equilibrium constant for the reactions
are:
k
H3PO4
H2PO4–
HPO42–
1
H+ + H2PO4–;
k2
k3
K1
H+ + HPO42–;
K2
H+ + PO43–;
K3
The equilibrium constant for
N3PO4
Raising the temperature of a reversible
chemical reaction:
(a) Favours the forward rate only
(d) Increases with time
1.
2.
In an equilibrium reaction, if ∆G° = 0 the
equilibrium constant, K should be equal to:
(a) temperature and pressure
(c) Is independent of time
62.
SO2 (g) + Cl2 (g)
(c) CaO is removed
(b) Decrease with time
61.
2NH3 (g)
(b) CO2 escapes out
(a) Is zero
60.
2NO (g)
PCl3 (g) + Cl2 (g)
(c) N2 (g) + 3H2 (g)
In lime kiln, the reversible reaction,
CaCO3 (s)
59.
(a) N2 (g) + O2 (g)
For
the
reaction
equilibrium,
2NOBr (g)
2NO (g) + Br2 (g), If PBr = P/9
2
at equilibrium and P is total pressure. The
ratio Kp/P is equal to:
3H+ + PO43– will be:
(a) K1/K2 K3
(b) K1 × K2 × K3
(c) K2/K1 K3
(d) K1 + K2 + K3
In which of the following equilibrium, change
in volume of the system does not alter the
number of moles?
67.
68.
PCl5 (g),
For reaction PCL3(g) + Cl2(g)
the value of K c at 250ºC is
26 mol litre –1 . The value of K p at this
temperature will be:
(a) 0.61 atm–1
(b) 0.57 atm–1
(c) 0.83 atm–1
(d) 0.46 atm–1
In which of the following cases, does the
reaction go furthest to completion?
(a) K = 103
(b) K = 10–2
(c) K = 10
(d) K =1
If K1 and K2 are the respective equilibrium
constants for the two reactions,
XeF6(g) + H2O(g)
XeO4(g) + XeF6(g)
XeOF4(g) + 2HF(g)
XeOF4(g) + XeO3F2(g)
The equilibrium constant for the reaction,
XeO4(g) + 2HF(g)
XeO3F2(g) + H2O(g) is:
(a) K1K 2
(b) K1/K22
(c) K2/K1
(d) K1/K2
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PHYSICAL CHEMISTRY
69.
70.
If 1.0 mole of I2 is introduced into 1.0 litre flask
at
1000
K,
at
equilibrium
(Kc = 10–6), which one is correct?
(a) [I2 (g)] > [I (g))]
(b) [I2 (g)] < [I (g)]
(c) [I2 (g)] = [I (g)]
(d) [I2 (g)] = 1/2[I(g)]
75.
A
B;
Kc =2
B
C;
Kc = 4
C
D;
Kc = 6
(a) K1 / K2
(c) K1K2
76.
D is:
(a) (2 + 4 + 6)
(b) (2 × 4)/6
(c) (4 × 6)/2
(d) 2 × 4 × 6
77.
For a reaction in equilibrium:
(a) There is no volume change
(d) The forward reaction is faster than
reverse reaction
73.
(a) Negative
(b) Positive
(c) Zero
(d) Undefined
(b) 2O3 (g)
3O2 (g)
(c) C(graphite)
C
74.
CO2(g) is:
(a) RT
(b) 1/√RT
(c) √RT
(d) 1
Consider the following equilibrium in a closed
container:
2NO2 (g)
(c) Kp Changes, but α does not changes
(d) Kp does not changes, but α changes
78.
At constant temperature, the equilibrium
constant (Kp) for the decomposition reaction.
N2O4
2NO2 is expressed by,
(4x2 P)
(1 – x )
Kp = ––––––––––
2
2SO3 (g)
Where P = pressure, x = extend of
decomposition. Which of the following
statement is true?
H2O (g)
(a) Kp increases with increase of P
An example of reversible reaction is:
(b) Kp increases with increase of x
(a) AgNO3(aq) + HCl(aq) ––––→ AgCl(s) + HNO3(aq)
(c) Kp increases with decrease of x
(b) 2Na + 2H2O ––––→ 2NaOH + H2
(c) NaOH + CH3COOH ––––→ CH3COONa + H2O
(d) Pb(NO3)2 + 2NaI ––––→ PbI2 + 2NaNO3
1.
2.
CO(g) + 1/2 O2(g)
(b) Both Kp and α change
(diamond)
(d) H2 (g) + 1/2 O2 (g)
Kp / Kc for the reaction,
(a) Neither Kp nor α change
Increase in temperature favours the forward
reaction in:
(a) 2SO2 (g) + O2 (g)
(d) K12K 2
At a fixed temperature, the volume of the
reaction container is halved. For this change,
which of the give statements holds true
regarding the equilibrium constant (Kp) and
degree of dissociation (α)?
(c) The rate of forward reaction is equal
to the rate of backward reaction
In a flask colourless N2O4 is in equilibrium
with brown coloured NO2. At equilibrium,
when the flask is heated at 100ºC the brown
colour deepens and on cooling it becomes
less coloured. The change in enthalpy ∆H,
for the system is:
(b) K1K 2
2
N2O4 (g)
(b) The reaction has stopped completely
72.
The equilibrium constant for the reactions,
+
O 2 (g)
2NO(g),
N 2 (g)
NO(g) + 1/2 O2 (g)
NO2 (g) are K1 and K2
respectively. Then the equilibrium constant
for
the
equilibrium
N2(g) + 2O2 (g)
2NO2 (g) is:
For the reactions,
Kc for the reaction, A
71.
By: Shailendra Kumar
(d) Kp remains constant with change in P or x
79.
In which of the following reaction increase in
pressure at constant temperature does not
affect the moles at equilibrium?
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PHYSICAL CHEMISTRY
(a) 2NH3 (g)
N2(g) + 3H2 (g)
(b) C (g) + 1/2 O2 (g)
CO (g)
Equilibrium constants K 1 and K 2 for the
following equilibria are related as:
(c) H2 (g) + 1/2 O2 (g)
H2O (g)
NO (g) + 1/2 O2 (g)
(d) H2 (g) + I2(g)
80.
81.
By: Shailendra Kumar
85.
2NO2 (g)
2HI (g)
For the reaction:
CO(g) + 1/2 O2(g)
CO2 (g), Kp / Kc is:
(a) RT
(b) (RT)–1
(c) (RT)–1/2
(d) (RT)1/2
The exothermic formation of ClF 3 is
represented by the equation:
Cl2 (g) + 3F2 (g)
86.
1
(b) K2 = –––––
K1
(c) K2 = K12
K1
(d) K2 = –––––
2
For the reaction,
CO2 (g) + 2H2O(l),
∆rH = –170.8 kJ mol–1
Which of the following will increase the
quantity of ClF3 in equilibrium mixture of Cl2,
F2 and ClF3?
Which of the following statements is not true?
(a) Increasing the temperature
(b) The reaction is exothermic
(b) Removing Cl2
(c) At equilibrium, the concentrations of
CO2(g) and H2O (l) are not equal
(a) Addition of CH 4 (g) or O 2 (g) at
equilibrium will cause to the right
(d) the equilibrium constant for the
reaction is give by
For the reaction :
2NO2(g)
[CO2]
Kp = –––––––––––
[CH4] [ O2]
2NO(g) + O2 (g); Kc = 1.8 × 10–6 at
–1
–1
184ºC and R = 0.083 JK mol . When Kp
and Kc are compared at 184ºC. It is found
that:
(a) Kp > Kc
(c) Kp = Kc
(b) Kp < Kc
< Kc
(d) Kp >
The graph relates In K eq vs (1/T) for a
reaction. The reaction must be:
(a) exothermic
InKeq
(b) Endothermic
(c) ∆H is negligible
(d) Highly spontaneous at
ordinary temperature
84.
1
(a) K2 = –––––
K12
2ClF3; ∆H = –329 kJ
(d) Adding F2
83.
2NO (g) + O2 (g); K2
CH4 (g) + 2O2 (g)
(c) Increasing the volume of container
82.
NO2 (g); K1
87.
Phosphorus pentachloride dissociates as
follows, in a closed reaction vessel,
PCl5(g)
PCl3 (g) + Cl2 (g)
If total pressure at equilibrium of the reaction
mixture is P and degree of dissociation of
PCl5 is x, the partial pressure of PCl3 will be:
x
(a) –––––– P
x+1
2x
(b) –––––– P
1–x
x
(c) –––––– P
x–1
x
(d) –––––– P
1–x
1/T
When two reactants A and
B are mixed to give products C and
D, the reaction quotient, Q at the initial stages
of reaction:
(a) is zero
(b) decreases with time
(c) independent of time
(d) increases with time
1.
2.
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PHYSICAL CHEMISTRY
A
By: Shailendra Kumar
n
s
w
e
r
s
01.
a
30.
a
59.
a
02.
d
31.
a
60.
d
03.
d
32.
c
61.
b
04.
b
33.
b
62.
a
05.
b
34.
b
63.
b
06.
a
35.
d
64.
a
07.
a
36.
a
65.
c
08.
b
37.
d
66.
a
09.
b
38.
b
67.
a
10.
b
39.
d
68.
c
11.
c
40.
a
69.
a
12.
c
41.
c
70.
d
13.
a
42.
b
71.
c
14.
c
43.
a
72.
b
15.
b
44.
b
73.
c
16.
a
45.
d
74.
c
17.
c
46.
c
75.
c
18.
d
47.
b
76.
b
19.
d
48.
b
77.
d
20.
d
49.
a
78.
d
21.
a
50.
b
79.
d
22.
a
51.
c
80.
c
23.
b
52.
a
81.
d
24.
a
53.
a
82.
a
25.
d
54.
a
83.
a
26.
a
55.
b
84.
d
27.
c
56.
b
85.
a
28.
a
57.
b
86.
d
29.
d
58.
b
87.
a
1.
2.
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